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What will be the pH of 0.05M barium hydr...

What will be the pH of `0.05`M barium hydroxide solution ?

A

`8`

B

`9`

C

`7`

D

`13`

Text Solution

Verified by Experts

Barium hydroxide is a strong electrolyte, i.e., it dissociates completely:
`Ba(OH)_(2)(aq.)rarr Ba^(2+)(aq.)+2OH^(-)(aq.)`
According to the equation,
`C_(OH^(-))=2C_(Ba(OH)_(2))=(2xx0.05)M`
`=0.1M`
`=10^(-1)M`
`:. C_(OH^(-))= 10^(-pOH)M`
We have
`pOH = 1`
For any aqueous solution at 298 K, we have
`pH+pOH=14`
`pH=14-pOH`
`=14-1`
`=13`
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Knowledge Check

  • The pH of 0.1 M ammonium hydroxide is

    A
    `14`
    B
    `lt 13`
    C
    `gt 13`
    D
    `lt 7`

  • What will be the pH value of 0.05 M Ba(OH)_(2) solution

    A
    12
    B
    13
    C
    1
    D
    12.96

  • 50 mL of H_(2)O is added to 50 mL of 1 xx 10^(-3)M barium hydroxide solution. What is the pH of the resulting solution?

    A
    `3.0`
    B
    `3.3`
    C
    `11.0`
    D
    `11.7`

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